
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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6. Use the molar volume of an ideal gas at STP to determine the volume (in mL) of 0.500 g of fluorine gas at STP.
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- (b) Consider the reaction between nitrogen gas and hydrogen gas to produce ammonia gas at STP. Infer the volume of hydrogen gas needed to produce 0.4 L of ammonia gas.arrow_forwardA gas sample at STP contains 4.28 g of ammonia gas, NH3. What is the volume of the ammonia gas?arrow_forwardOne mole of hydrogen gas has a mass of 2.02 g. Use your value of the molar volume of hydrogen to calculate the mass of one liter of hydrogen gas at STP. This is the density ofarrow_forward
- 12. Suppose 435 mL of Ne gas at 21 °C and 1.09 atm, and 456 mL of SF6 at 25 °C and 0.89 atm are put into a 325 mL flask at 30.2 °C. (a) What will be the total pressure in the flask? (b) What is the mole fraction of for each of the gases in the flask? (c) How many grams of each gas are in the flask?arrow_forwardCalculate the density of CO2 in g / L , at STP. Calculate number of moles of gas that occupies a volume of 1.75 Larrow_forwardLithium metal reacts with nitrogen gas to make the compound lithium nitride. What mass of lithium metal reacts completely with 58.1 mL of nitrogen gas at STP?arrow_forward
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